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Will the molar mass of 0.500g aspirin differ than the molar mass of .900g aspirin? Will the molar mass of 0.500g aspirin differ than the molar mass of .900g aspirin? My instructor stated that it does not matter but I'm still doubting, so thanks to everyone who helped to answer my curiosity. Thanks, billy S.

billy S replied: "Think of 1 Litre of water, it weighs 1 kg Even if you had only 200 ml of water, an entire 1 Litre still weighs 1 kg If you have 600 ml of water, 1 L will still weigh 1 kg The molar mass is the mass of 1 mole of a molecule. 1 mole is a unit of measurement, (like a Litre is a measurement of volume) A mole is the amount of a substance that contains 6.022 x 10^23 molecules. Since there is alway the same number of a molecule in 1 mole then 1 mole will always have the same mass. The number of moles will be different and the mass is obviously different, but the molar mass is constant."

Calculate the molar mass of a aspirin tablet that contains 500.0 mg of C9H804.? Calculate the molar mass of a aspirin tablet that contains 500.0 mg of C9H804. Does the 500.0mg (0.500g) effected the molar mass? If it does, will it be something like this? molar mass = 0.500g/# of moles in C9H804. Thanks, Paul B. I did it that way already and I was just making sure it was right. You're great. :-)

Paul B replied: "You calculate the molar mass of aspirin from the molecular formula. Do you mean, calculate the number of moles of aspirin in the tablet? If so, just divide the mass (g) of aspirin in the tablet by the molar mass (g/mole) to get your answer in moles."

Titration of Aspirin. Whats the molar mass? Im stumped!? Did and experiment in lab on the titration of 325mg aspirin with 0.100 M of NaOH. I did this experiment twice so their fore Im looking for the average molar mass. Trail one I used 18.8 of NaOH and Trail 2 I used 18.4. I think the equation I would use is molar mass= grams/mole. I just dont know how to apply. HELP!

bernie_bph replied: "From the data you provided, calculate the number equivalents of aspirin. equivalents of aspirin = (0.1)(0.0188) = 0.00188 If you did not dilute your aspirin, below is your result: trial 1 = (325/1000)/(0.00188) = 172.872 grams/mole trial 2 = (325/1000) / 0.00184 = 176.630 grams/mole average = 174.751 grams/mole from source: aspirin has a molar mass of = 180.157 g/mol"

what is the percentage by mass of aspirin in the tablet? aspirin c9h8o4 has a molar mass of 100g per mole. 1 mole of asprin reacts with one mole of NaOH. a tablet of a painkiller has a mass of .483g and is known to contain aspirin. the tablet reacts with exactly 16.65 cm^3 of .100 mol per liter of NaOH.

peter r replied: "moles of NaOH = M V =.1 * 16.65 = 1.655 *10^-3 moles the problem says these moles react equally with the asprin so moles of aspirin = 1.655 *10^-3 moles mass of aspirin = #moles * MW = 1.6655* 10^-3 *180.16 = ,3g in the tablet we have .3/.483 = 62.11% I'm not sure where the 100 g/ mole come from. I think it is an error. If not you can substitute it for the 180.16 I have used and recalculate. aspirin is acetylsalicylic acid which has a MW of180.16 !"

Which is the molar mass of acetylsalicylic acid (aspirin) C9H8O4 ? A. 29 g B. 108 g C. 180 g D. 196 g

rmjrenneboog replied: "at wt of C = 12 at wt of O = 16 at wt of H = 1 Multiply each by how many there are and add them together. You should be able to do this in your head..."

ahmed b replied: "THANKS .really Idonot remember, But if you know please answer"

SOS20 replied: "C= 108+8+64"

Raoul S. Tickler replied: "C = 12 H = 1 O = 16 Work it out"

skipper replied: "9x12.011+8x1.0079+4x15.9994 = 180.1598 C. 180 g"

John F replied: "Go to your periodic table and take all the masses down: H = 1g O = 16g C = 12g Now you have 9 carbons, 8 hydrogens and 4 oxygens so: H8 = 8g O4 = 64g C9 = 108g Add them all up to get the molar mass: 8 + 64 + 108 = 180g Answer is C. I hope I helped."

Matt K replied: "Carbons atomic mass is 12.01 amu of g/mol Hydrogens atomic mass is 1.008 amu or g/mol Oxygens atomic mass is 16.00 amu or g/mol So (12.01 x 9) + (1.008 x 8) + (16.00 x 4) = 180.15 = C. 180 g"

Professor Moose replied: "Not sure why some of these have been given a thumbs down but the answer definitely is (c) and Matt K's answer explains it perfectly!"

Aspirin is produced by the reaction of salicyclic acid? Aspirin is produced by the reaction of salicyclic acid (molar mass = 138.1 g mol-1) and acetic anhydride (molar mass 102 g/mol) 2C7H6O3(s) + C4H6O3(l) 2C9H8O4(s) + H2O(l) If you mix 100 g of each of the reactants, how many grams of aspirin (molar mass 180.16 g/mol) can be theoretically obtained?

Halck replied: "First you find your limiting reactant by calculating tho moles of each. As they react 2-to-1 it should be quite easy. If you have less salicyclic acid than twice the amount of acetic anhydride, the salicyclic acid is the limiting reactant. If salicyclic acid is the limiting reactant you get just as many moles of Aspirin as you have of salicyclic acid. If acetic anhydride is the limitng reactant you get twice as many moles of Aspirin. Then You calculate the mass of Aspirin from the number of moles. Equations needed: n=m/M m=n*M"

What is the number of moles of each atom in one mole of aspirin? What is aspirin's molar mass?

Dr.A replied: "The formula of aspirin ( acetyl salycilic acid ) is C9H8O4 Molar mass = 180.16 g/mol 1 Mole of aspirin => 9 moles C , 8 moles O and 4 moles O"

How do I find Molecular Weight from molar mass? I have found the molar mass of the aspirin I made and it is 172.07 but the lab book says to calculate the molecular weight. Are they the same? I found the molar mass from titration. I took the L of NaOH and multiplied it by the molarity of NaOH times the mole fraction of aspirin/NaOH to get moles of aspirin. Then I divided mass of aspirin used by the moles of aspirin to get 'molar mass. Is it the same as molecular weight?

eEeEe replied: "Molar mass and molecular weight are interchangeable terms. So yes, they are the same thing."

Molar mass, concentration, grams...? The concentration of acetylsalicylic acid (aspirin C9H8O4 with molar mass of 180. g/mol) in your plasma is found to be 2.99 x 10^-4 M after you take two tablets of aspirin. If the volume of your plasma is 5.85 L, how many grams of aspirin are in your blood?

Rebecca Okay replied: "Molarity = number of moles ÷ Volume M = n ÷ V 2.99 x 10^4 mol/L = n ÷ 5.85L Solve for n Then take number of moles and multiply by gram molecular mass to get the number of grams. n x GMM = m n x 180 = m"

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